Login
Login
Login
Register

Tutor HuntTest QuestionsChemistry QuestionsYear 10 Chemistry Questions

 

Mass Changes When A Reactant Or Product Is A Gas (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Mass Changes When A Reactant Or Product Is A Gas' from the broader topic Quantitative Chemistry. The test is geared towards the AQA exam board style syllabus.
Start Test
Incorrect: 0
Correct: 0
Question 1
...
Congratulations - you have completed the test!
Your final score was

Below a typical questions that will be covered in this test. You final score will be logged on your account

A student collects gas from a reaction into an inverted measuring cylinder but fails to fill the trough with water high enough so some gas escapes. How will the experimentally measured mass change compare with the theoretical mass change?
Which experimental change will make the measured mass decrease during a reaction more accurately reflect the mass of gas evolved rather than being underestimated?
A reaction produces gas that is dissolved in the liquid rather than escaping. If later the liquid is heated and gas evolves, what will an open-balance measurement show while gas is dissolved and then after heating?
Which method ensures the mass of a reacting system remains constant during a reaction that produces gas so students can easily demonstrate conservation of mass?
Complete the stoichiometric calculation: 5.00 g of Na2CO3 reacts fully with acid producing CO2. How many grams of CO2 are produced? (Mr Na2CO3 = 106, CO2 = 44).
A container initially contains 1.00 g of hydrated copper sulfate. After heating to drive off water the mass is 0.64 g. What mass of water was lost?
A sample of 11.7 g of hydrated copper sulfate changes to 2.99 g anhydrous CuSO4 and 1.47 kJ of energy is absorbed when 4.68 g of hydrate changed to 2.99 g anhydrous. Using these ratios, calculate the maximum mass of water that can be produced from 11.7 g of hydrated copper sulfate. (Use proportional scaling.)
1.00 g of magnesium is burned in oxygen to make magnesium oxide. (Ar: Mg = 24.3, O = 16.0) What is the increase in mass of the sample due to oxygen combining with the magnesium?
A student wants to demonstrate conservation of mass for a reaction that produces CO2. Which setup will best show no mass change?
A student reacts 2.00 g of zinc with excess hydrochloric acid in an open flask (Zn ? Zn2+ + 2 e-; reaction produces H2 gas). Using Zn Ar = 65.4, how much mass is lost from the system when the reaction produces hydrogen gas? (Give an approximate value.)
When 1.00 g of carbon is completely oxidised to CO2 (oxygen supplied from air), by how much does the mass of the carbon sample increase? (Ar C = 12, O = 16)